In a gydrogen - oxygen fuel cell, `67.2` litre of `H_(2)` at S.T.P is used in 5 min. What is the average current produced?

Options

A. ` 549.4` amp
B. `643.33` amp
C. 965 amp
D. 1930 amp

Explanation

To find the average current produced in a hydrogen-oxygen fuel cell when `67.2` liters of `H₂` is used in `5` minutes, we can follow these steps:

### Step 1: Calculate the total charge produced from the volume of hydrogen gas used.

At standard temperature and pressure (STP), `22.4` liters of hydrogen gas produces `19300` coulombs of charge. We need to find out how much charge is produced from `67.2` liters of hydrogen.

Using the proportion:
\[ \text{Charge from } 67.2 \text{ liters} = \left( \frac{19300 \text{ C}}{22.4 \text{ L}} \right) \times 67.2 \text{ L} \]

### Step 2: Perform the calculation.

\[ \text{Charge} = \frac{19300 \times 67.2}{22.4} \]

Calculating this gives:
\[ \text{Charge} = \frac{19300 \times 67.2}{22.4} = 579000 \text{ C} \]

### Step 3: Calculate the average current.

Current (I) can be calculated using the formula:
\[ I = \frac{Q}{t} \]
where \( Q \) is the total charge and \( t \) is the time in seconds.

Given that the time is `5` minutes, we convert this to seconds:
\[ t = 5 \text{ min} \times 60 \text{ s/min} = 300 \text{ s} \]

Now substituting the values:
\[ I = \frac{579000 \text{ C}}{300 \text{ s}} = 1930 \text{ A} \]

### Conclusion

The average current produced is **1930 Amperes**.

---